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The solubility product of a salt having general formula MX2, in water is 4x10-12. The concentration of M2+ ions in the aqueous solution of the salt is - [AIEEE-2005]
- a)1.0 x 10-4
- b)2.0 x 10-6 M
- c)4.0 x 10-10 M
- d)1.6 x 10-4 M
Correct answer is option 'A'. Can you explain this answer?
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The solubility product of a salt having general formula MX2, in water ...
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The solubility product of a salt having general formula MX2, in water ...
To solve this problem, we need to use the concept of solubility product (Ksp) and the stoichiometry of the salt.
The general formula of the salt is MX2, which means that for every molecule of salt that dissolves in water, it will dissociate into one M2+ ion and two X- ions.
Let's assume that the initial concentration of the salt (MX2) is "s". After complete dissociation, the concentration of M2+ ions will be "s" and the concentration of X- ions will be "2s".
The solubility product expression for this salt can be written as:
Ksp = [M2+][X-]^2
Given that the solubility product (Ksp) of the salt is 4x10^-12, we can substitute the concentrations of the ions and the value of Ksp into the equation:
4x10^-12 = (s)(2s)^2
4x10^-12 = 4s^3
s^3 = 10^-12
s = (10^-12)^(1/3)
s = 10^-4
Therefore, the concentration of M2+ ions in the aqueous solution of the salt is 1.0 x 10^-4 M.
Hence, the correct answer is option A, 1.0 x 10^-4 M.
The general formula of the salt is MX2, which means that for every molecule of salt that dissolves in water, it will dissociate into one M2+ ion and two X- ions.
Let's assume that the initial concentration of the salt (MX2) is "s". After complete dissociation, the concentration of M2+ ions will be "s" and the concentration of X- ions will be "2s".
The solubility product expression for this salt can be written as:
Ksp = [M2+][X-]^2
Given that the solubility product (Ksp) of the salt is 4x10^-12, we can substitute the concentrations of the ions and the value of Ksp into the equation:
4x10^-12 = (s)(2s)^2
4x10^-12 = 4s^3
s^3 = 10^-12
s = (10^-12)^(1/3)
s = 10^-4
Therefore, the concentration of M2+ ions in the aqueous solution of the salt is 1.0 x 10^-4 M.
Hence, the correct answer is option A, 1.0 x 10^-4 M.
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The solubility product of a salt having general formula MX2, in water is 4x10-12. The concentration of M2+ ions in the aqueous solution of the salt is - [AIEEE-2005] a)1.0 x 10-4b)2.0 x 10-6 Mc)4.0 x 10-10 Md)1.6 x 10-4 MCorrect answer is option 'A'. Can you explain this answer?
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